Calculate the percent composition of the following elements
This is like Percent Yield, but you divide the part of the weight of each element by the total weight of the molecule. Then times it by 100.
Example - H2O.
Total mass = 18.015 g.
2 Hydrogens mass = 2.016 g. %H = (2.016/18.015)(100)=11.19%
1 Oxygen mass = 15.999 g. %O = (15.999/18.015)(100)=88.81%
I know its right because they add up to 100%
Write the percent sign.
1) CuBr2
2) NaOH
3) (NH4)2S
4) N2S2
5) NH4BrO4
Limiting Reagent Worksheet divide the question amount by the equation amount. Convert to grams before you divide. Whichever is the smallest number is the limiting reagent.Use the equation P4O10 + 6 H2O→ H3PO4 below
6) If you had 100 g of both reactants, which would be the limiting reagent?7) If you react 50 g of the first reactant with 100g of the second, which would be the limiting reagent?8) if you combine 1000 g of the first reactant with 100 g of the second reactant, which is the limiting reactant? Test Review Questions 9) What is the molar mass of H2SO4? (how many grams does it weigh?)10) How much does 3.5 moles of H2SO4 weigh? (Remember that 1 mol = the molar mass (add it up from the Periodic Table).11) How many molecules are in 2.4 moles of H2SO4? (remember 1 mol = 6.022 x 1023 molecules)12) How many Liters does 3.2 moles of H2SO4 as a gas occupy? (remember 1 mol = 22.4 L) Use the equation 8 Fe + S8 → 8 FeS below 13) How many grams of FeS are produced by 15 g of Fe?14) If FeS was a gas how many Liters would be produced by 15 g of Fe?15) If you had 100 grams of Fe and 200 g of S8, which would be the limiting reagent? (remember to divide the question amount by the equation amount. Convert to grams before you divide. Whichever is the smallest number is the limiting reagent.)16) what is a limiting reagent?17) What did you use to calculate the empirical formula? (look at the title of the chart from the project on 14-5)
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Percent Composition Worksheet
- Write the percent sign.
1) CuBr22) NaOH
3) (NH4)2S
4) N2S2
5) NH4BrO4
Limiting Reagent Worksheet
divide the question amount by the equation amount. Convert to grams before you divide. Whichever is the smallest number is the limiting reagent. Use the equation P4O10 + 6 H2O → H3PO4 below
6) If you had 100 g of both reactants, which would be the limiting reagent?7) If you react 50 g of the first reactant with 100g of the second, which would be the limiting reagent?8) if you combine 1000 g of the first reactant with 100 g of the second reactant, which is the limiting reactant?
Test Review Questions
9) What is the molar mass of H2SO4? (how many grams does it weigh?)10) How much does 3.5 moles of H2SO4 weigh? (Remember that 1 mol = the molar mass (add it up from the Periodic Table).11) How many molecules are in 2.4 moles of H2SO4? (remember 1 mol = 6.022 x 1023 molecules)12) How many Liters does 3.2 moles of H2SO4 as a gas occupy? (remember 1 mol = 22.4 L)
Use the equation 8 Fe + S8 → 8 FeS below
13) How many grams of FeS are produced by 15 g of Fe?14) If FeS was a gas how many Liters would be produced by 15 g of Fe?15) If you had 100 grams of Fe and 200 g of S8, which would be the limiting reagent? (remember to divide the question amount by the equation amount. Convert to grams before you divide. Whichever is the smallest number is the limiting reagent.)16) what is a limiting reagent?17) What did you use to calculate the empirical formula? (look at the title of the chart from the project on 14-5)